Chem 101 Assignments Test II
Which quantum state (n, l, ml) is NOT possible?
(3, 0, 1)
What is the energy of a mole of photons that have a wavelength of 779 nm?
1.537 x 10^5 J
What is the energy of light that must be absorbed by a hydrogen atom to transition an electron from n=3 to n=7?
1.98 x 10^-19 J
The bond dissociation energy to break 3 bond(s) in 1 mole of CH4 molecules is
1233 kJ
Which of the following represents the electron configuration of P3-?
1s2 2s2 2p6 3s2 3p6
What is the electron configuration of Co2+?
1s2 2s2 2p6 3s2 3p6 3d7
The ground state of electron configuration of a Se atom is
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4
Which of the following electron configurations represent a transition metal atom?
1s2 2s2 2p6 3s2 3p6 4s2 3d7
How many core electrons does an atom of Beryllium contain?
2
What is the maximum number of electrons that can have following set of quantum numbers? n=2, l=1, ml=1
2
Iron has a work function of 4.50 eV. What is the longest wavelength of light that will cause the ejection of electrons?
276 nm
For which atomic orbital does n=3 and l=1?
3p
What is the wavelength of blue light that has a frequency of 6.41 x 10^14 s^-1?
4.68 x 10^2 nm
The bond dissociation energy to break 1 hydrogen-carbon bond(s) in 1 mol of HC(triple bond)CH molecules is
411 kJ
Which of the orbital electron configurations is not possible?
4p7
Which of the following electronic transitions represents an increase in energy in a multi-electron atom?
4s -> 3d
How many orbitals are allowed in the subshell when l=2?
5
A photon has a frequency of 8.15 x 10^8 Hz. What is the energy of this photon?
5.40 x 10^-25 J
What is the frequency of green light that has a wavelength of 507 nm?
5.92 x 10^14 s^-1
Determine the energy of a photon with a wavelength of 307 nm.
6.47 x 10^-19 J
Which of the following pairs of ions represent isoelectronic species?
Al3+ and O2-
Which color (frequency) of light travels the fastest in a vacuum?
All have the same speed
Based on their positions in the periodic table, which of the following bonds is the most polar?
B-F
What scientist proposed that the electron in a hydrogen atom can only have certain energies?
Bohr
Which element has the ground state electron configuration [Ar] 4s2 3d10 4p5?
Br
Based on their positions in the periodic table, which of the following bonds is the most polar?
C-F
Write the chemical formula for oxalic acid
C2 H2 O4
Write the chemical formula for aluminum acetate
C6 H9 AlO6
Write the chemical formula for calcium chloride
Ca Cl2
Which atom in the molecule ClF would have a partial positive charge?
Cl
Which element has the electron configuration 1s2 2s2 2p6 3s2 4s1 3d5?
Cr
The energy released in the reaction: F(g) + e- -> F-(g) is known as the
Electron Affinity
What element is designated by the orbital diagram below?
F
Rank the following atoms in order of decreasing first ionization energies (i.e highest to lowest): li, Be, Ba, F
F > Be > Li > Ba
All of the following pairs of ions are isoelectronic except which one?
Fe2+ and Mn3+
Which element has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2?
Ge
Which of the following is an example of a covalent bond?
H-Cl
Write the chemical formula for chlorous acid
HClO2
Which scientist surmised the scientific principle that the position and momentum of an electron cannot be known simultaneously with a high degree of accuracy?
Heisenberg
What quantum mechanics principle states that electrons are added to atomic orbitals with the same energy so that each orbital is singularly occupied with electrons having same spin?
Hund's Rule
What quantum mechanics principle states that electrons are added to atomic orbitals with the same energy so that each orbital is singularly occupied with electrons having the same spin?
Hund's Rule
Excited hydrogen atoms emit radiation in which region(s) of the electromagnetic spectrum?
IR, visible, and UV
Which of the following radii comparisons is correct?
In3+ , In+
Which periodic trend quantifies the amount of energy required to remove an electron from a neutral, gaseous atom?
Ionization Energy
A student draws the orbital diagram below for the 3d electrons in a V atom. What, if anything is incorrect about the drawing?
It violates Hund's Rule
A student draws the orbital diagram below for the 3d electrons in an V atom. What, if anything, is incorrect about the drawing?
It violates Hund's Rule
A student draws the orbital diagram below for the 3p electrons in an S atom. What, if anything, is incorrect about the drawing?
It violates Hund's rule
Which is the following is an example of an ionic bond?
K-F
What is the noble gas core in the electron configuration for Ru?
Kr
Which of the following atoms would have the longest de Broglie wavelength, if all have the same velocity?
Li
Which of the following electron configurations is incorrect?
Mn [Ar] 4s2 4d5
Which of the following atoms below has/have five valence electrons?
N
Write the chemical formula for ammonium thiocyanate
NH4 SCN
Valence electrons in which of the following atoms experience the greatest effective nuclear charge (Zeff)?
Ne
What element is designated by the orbital diagram below?
Ni
Rank the following atoms in order of increasing size (i.e smallest to largest): Li, Al, Be, Ba, O
O < Be < Li < Al < Ba
Write the chemical formula for tetraphosphorous hexasulfide
P4 S6
Write the chemical formula for phosphorous trihydride
PH3
Which of the following states that no two electrons can have the same set of four quantum numbers?
Pauli Exclusion Principle
What is the noble gas core in the electron configuration for U?
Rn
Who developed the equation that allowed the energy of the electron to be described quantum mechanically?
Schrodinger
Which of the following metals would be expected to have the smallest atomic radius?
Tantalum (Ta)
Which of the following statements is FALSE?
The bond between the carbons in the molecule H2C=CH2 is stronger than the bond between the carbons in HC(triple bond)CH
True or false: two electrons can simultaneously occupy the same (n,l,ml) orbital.
True
Which of the following has the electron configuration 1s2 2s2 2p6 3s2 3p6 3d3?
V2+
Light wave A has a greater frequency than light wave B. Which has a greater wavelength?
Wave B
Which of the following is the electron configuration for Mn?
[Ar] 4s2 3d5
Which of the following is the electron configuration for Ba?
[Xe]6s2
If light has a lot of energy, it will have:
a small wavelength
Which of the following has the shortest bond length?
a triple bond
Which of the following is the strongest type of bond?
a triple bond
IUPAC name for Al2S3
aluminum sulfide
IUPAC name for BaI2
barium iodide
IUPAC name for CaBr2
calcium bromide
IUPAC name for CrBr3
chromium (III) bromide
IUPAC name for CuS2
copper (I) sulfide
The trend towards smaller atomic radii as one moves to the right in a period is ________
due to the effective nuclear charge increasing
Which particle would have the longest de Broglie wavelength traveling with the same velocity?
electron
Which of the following statements best describes electronegatively in atoms?
electronegativity is the attraction an element's nucleus has for the electrons in a chemical bond
What happens to the energy of a photon if the wavelength is doubled?
energy is reduced by one-half
Which of the following forms of radiation has the highest frequency?
gamma rays
Which of the following forms of radiation has the shortest wavelength?
gamma rays
What is observed when a noble gas is heated and the emitted light shone through a prism?
individual lines of varying colors
IUPAC name for FeCl3
iron (III) chloride
Given a particular value of the principal quantum number (n), which quantum number primarily determines the shape of an orbital?
l
Red light has a _____ frequency and a _______ wavelength than ultraviolet rays.
lower, longer
Which of the following sets is NOT allowed?
n=2, l=2, ml=2
Which of the following sets of quantum numbers could describe an electron in the orbital shown below?
n=3, l=0, ml=0
Which of the following sets of quantum numbers can describe a 3p electron?
n=3, l=1, ml=1
An electron is shown to occupy a d orbital. Which of the following sets of quantum numbers can describe this electron?
n=3, l=2, ml=-2
Which of the following sets of quantum numbers is not allowed?
n=4, l=0, ml=-1
Which of the following sets of quantum numbers represents an electron with the highest energy in a multi-electron atom?
n=4, l=1, ml=1
A ground state atom of As could not have any electrons with which of the following configurations?
n=4, l=2, ml=0, ms=+1/2
If l=0, which of the following may be true?
n=6
In a polar covalent bond,
one atom in the bond must have higher electronegativity than the other atom
Which type of electromagnetic radiation has the largest wavelength?
radio waves
Photons are shone on a piece of metal and one electron is ejected for each absorbed photon. What happens when the wavelength of light is decreased?
the ejected electrons would have greater kinetic energy
In the photoelectric effect, if the intensity of light shone on a metal increases, what will happen?
there will be more electrons ejected
Which of the following best describes what happens when an ionic bond forms?
two atoms, one atom which is more electronegative than the other, exchange electrons and the charges hold the atoms together
A more electronegative atom
will have more attraction to the electrons in a chemical bond